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1. IONS
&
MOLECULES

2. IONS
• When a neutral
atom gains or
loses one or more
electrons, it
becomes
electrically
charged particle
called ion.
2

3. TYPES OF
IONS
1. Anion – atom
that gains electron
becomes
negatively
charged.
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4. 2. Cation – when
atoms gives off
an electron, its
charge becomes
positive.
4

5. • Monoatomic ions – ion that consists of only one atom.
Example: Na+, Mg2+, Fe3+, S2-, Cl-
• Polyatomic ions – an ion that contains more than one
atom.
Example: PO₄⁻³, OH⁻, NH₄⁺
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6. RULES IN NAMING IONS
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7. 7

8. 1.) ALKALI/ALKALINE EARTH METALS
• GROUP 1A – loses 1 electron only
Example: Na+ sodium
K+ potassium
• GROUP 2A – loses 2 electrons
Example: Mg2+ magnesium
Ca2+ calcium
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9. TRY!!!
•Write and name the ion formed by:
1. Lithium
2. Barium
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10. 2.) TRANSITION METALS
 ends with –ous (ion
with the lower charge)
 ends with –ic (ion with
higher charge)
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classical systematic
Fe2+ ferrous iron(II)
Fe3+ ferric iron(III)

11. 3. NONMETALS
• Nonmetals take a different nomenclature.
• The monoatomic anions are named by attaching the
suffix – ide to the first few letters(root) of the nonmetal name.
Ex. Br - bromide
S2- sulfide
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12. TRY!!!
•Write and name the ions formed by:
1. OXYGEN
2. FLUORINE
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13. 4. NONMETALS (POLYATOMIC IONS
WITH OXYGEN)
• Ends with –ite (the anion with lesser oxygen)
• Ends with –ate (the anion with more oxygen)
• Example:
NO2
- nitrite
NO3
- nitrate
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14. 5. HALOGENS
• Can form four(4) polyatomic ions with oxygen.
• Each ion is named differently depending on the number of
oxygen atoms present.
• 1 O atoms: CIO- hypochlorite
• 2 O atoms: CIO2
- chlorite
• 3 O atoms: CIO3
- chlorate
• 4 O atoms: CIO4
- perchlorate
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15. TRY!!!
• Write and name the four anions of BROMINE
and OXYGEN.
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16. NAMING IONIC & MOLECULAR
COMPOUND
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17. IONIC COMPOUND
•A compound consist
of:
•1 metal (+)
•1 nonmetal (-)
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18. IONIC COMPOUND
(WITHOUT
TRANSITION METALS)
aluminum oxide
Al3+ O2-
Balance Charges
6+ 6-
Al2 O3
Chemical
Formula/Name
Al2O3
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19. IONIC COMPOUND (WITH A
TRANSITION METALS)
• Name of Transition Metal
• (Roman Numeral) – oxidation number
• Nonmetal ending in –ide
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iron (III) oxide
Fe3+ O2-
Balance Charges
6+ 6-
Fe2 O3
Chemical Formula
Fe2O3

20. POLYATOMIC ION
calcium phosphate
Ca2+ PO4
3-
Balance Charges
6+ 6-
Ca3 (PO4)2
Chemical Formula
Ca3(PO4)2
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21. IONIC COMPOUNDS WITH A
TRANSITION METAL & POLYATOMIC
ATOM
• Name of Transition Metal
• (Roman Numeral) – oxidation number
• Polyatomic atom
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copper (II) nitrate
Cu2+ NO3
-
Balance Charges
2+ 2-
Cu (NO3)2
Chemical Formula
Cu(NO3)2

22. MOLECULAR
COMPOUND
• Refers to covalent
compound.
• Covalent compound:
• 2 nonmetals (-)
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23. MOLECULAR
COMPOUND
PREFIXES:
1 – mono
2 – di
3 – tri
4 – tetra
5 – penta
6 – hexa
7 – hepta
8 – octa
9 – nona
10 – deca
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24. NAMING COVALENT COMPOUND
•DO NOT balance charges
•Prefix + name of nonmetal
•Prefix + nonmetal ending in –ide
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25. NAMING COVALENT
COMPOUND
Example:
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diphosphorus pentoxide P2O5

26. POLYATOMIC IONS
ammonium sulfate
+ 2-
NH4 SO4
Balance Charges
+2 -2
NH4 SO4
Chemical Formula
(NH4)2SO4
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27. OTHER COMPOUNDS
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28. HYDRATED SALTS
• Ionic compounds with water molecules (H2O)
• Greek prefix + hydrate
Example:
CuSO4 ● 5H2O Copper (II) sulfate pentahydrate
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29. ACIDS
• Compounds that give off hydrogen ions when dissolved in
water (aqueous)
• Anion name is prefixed with hydro- , suffixed with –ic and
added with the term acid.
• Example:
HCl(g) hydrogen chloride HCl(aq) hydrochloric acid
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30. TERNARY ACIDS
• A ternary acid forms from a polyatomic ions.
• -ite is replaced with –ous
• -ate is replaced with –ic
• Example:
NO2
- nitrite +H2O HNO2 nitrous acid
NO3
- nitrate +H2O HNO3 nitric acid
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